## 8.67

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Abigail Urbina 1K
Posts: 102
Joined: Thu Jul 27, 2017 3:01 am

### 8.67

I'm a little bit confused as to how the solution manual came up with the value of $\Delta H=$-242 kJ/mol in part a of 8.67. I understand that to find the enthalpy of the reaction, you need to use the equation of bonds broken-bonds formed. I still can't seem to get that same value though. Can someone show me how they came up with that delta H value in part a?

8.67 Use the information in Tables 8.3, 8.6, and 8.7 to estimate the enthalpy of formation of each of the following compounds in the liquid state. The standard enthalpy of sublimation of carbon is 717 kJ·mol 1. (a) H2O; (b) methanol, CH3OH; (c) benzene, C6H6 (without resonance); (d) benzene, C6H6 (with resonance).

Abigail Urbina 1K
Posts: 102
Joined: Thu Jul 27, 2017 3:01 am

### Re: 8.67

Update: found my mistake, I had an error in one of the digits

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